II. Bohr Model of the Atom (p )

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Presentation transcript:

II. Bohr Model of the Atom (p. 125-128) Ch. 5 - Electrons in Atoms C. Johannesson

A. Line-Emission Spectrum excited state ENERGY IN PHOTON OUT ground state C. Johannesson

B. Bohr Model e- exist only in orbits with specific amounts of energy called energy levels Therefore… e- can only gain or lose certain amounts of energy only certain photons are produced C. Johannesson

C. Johannesson

B. Bohr Model 6 Energy of photon depends on the difference in energy levels Bohr’s calculated energies matched the IR, visible, and UV lines for the H atom 5 4 3 2 1 C. Johannesson

C. Other Elements Helium Each element has a unique bright-line emission spectrum. “Atomic Fingerprint” Helium Bohr’s calculations only worked for hydrogen!  C. Johannesson

D. Bohr Practice Use the Bohr Model/EM Spectrum on p. 8 of your reference tables. What type of light is produced when an electron moves from n=4 to n=1? What wavelength is produced when an electron moves from n=3 to n=2? What color of light is number 2? Which has more energy: red light or violet light? Which has less energy: Radio waves or ultraviolet radiation? Which has a smaller wavelength green or infrared? C. Johannesson